Calculate the mass of barium hydroxide required to neutralize 50 g of nitric acid.

When nitric acid interacts with barium hydroxide, barium nitrate is formed. The chemical reaction is described by the following equation:

Ba (OH) 2 + 2HNO3 = Ba (NO3) 2 + 2H2O;

From one mole of barium hydroxide, one mole of barium nitrate is formed. This requires two moles of acid.

Let’s find the amount of substance in 50 grams of nitric acid.

Its molar mass is:

M HNO3 = 1 + 14 + 16 x 3 = 63 grams / mol;

The amount of the substance will be:

N HNO3 = 50/63 = 0.7936 mol;

Find the mass 0.7936 / 2 = 0.3968 mol of barium hydroxide.

M Ba (OH) 2 = 137 + (16 + 1) x 2 = 171 g / mol;

m Ba (OH) 2 = 0.3968 x 171 = 67.8528 grams;